History of Periodic T.
1. The Periodic Table
You should know the following by the end of
today’s class…
• History of the idea of elements including
the contributions of the Greeks, Boyle and
Davy and Moseley
• Symbols of elements 1–36.
• History of the periodic table, including the
contributions of Dobereiner and Newlands
• The differences between the first Periodic
table and the modern table
Definition
• An element is a substance that
cannot be broken down into a
simpler substance.
Examples of Elements
Carbon (C)
Sodium (Na)
Examples of Elements
Bromine (Br)
Gold (Au)
Examples of Elements
Aluminium (Al)
The most abundant
metal in the Earth’s
crust
Silver (Ag)
Examples of Elements
Chlorine (Cl)
Hydrogen (H)
Examples of Elements
Tin (Sn)
Platinum (Pt)
Question?
•But where did the idea
of these “elements”
first come from?
The Ancient Greeks
In particular Empedocles 490 – 435 BCE,
had the idea that there were four basic
building blocks (elements) from which
everything was made:
earth,
fire,
water
and air
IDEA THAT MATTER IS COMPOSED OF ELEMENTS AND THAT
DIFFERENT ELEMENTS COMBINE TO MAKE NEW THINGS!
The Ancient Greeks
Piece of matter
Split or break up
Democritus
Around 2500 years ago
Eventually I end up with something which
cannot be broken up – called an element
Robert Boyle
Irish
scientist,
Robert
Boyle,
later defined what
an element was:
An element is a substance that cannot
be broken down into any simpler substance
Robert Boyle
17th Century
Definition
Humphrey Davy
• Davy was an English chemist who started out
his research examining the medicinal effect of
various gases
Humphry Davy
Davy
used
electricity to split
up compounds to
form elements
Humphry Davy
19th Century
Davy’s Elemental Discoveries
1807
1808
Elements
• Elements are made up of only one type of atom.
Naming the elements
• After a planet ….mercury, uranium
• European mythological figures….Titanium after
the Titans
• After its colour…. Gold
• After a physical property… Bromine= bad smell
• After a country…. francium = France
• After yourself….?
• After a scientist… Es = Einsteinium
The elements song
• http://youtu.be/aPq3SEteEJc - YouTube
Recap
• What is an element?
• What did the ancient Greeks think
materials were made of?
• Who was Robert Boyle?
• What contribution did Davy make to the
knowledge of the elements?
Arrangement of the elements
• All of the known elements
of today are arranged on
….The Periodic Table of
Elements
Pictorial view of the Modern Periodic Table
Looking for a pattern in the
elements
• In the 1800s over 50
elements had been
discovered and more
were being found!
• Chemists wanted to
find if there was any
pattern to the elements
Date of Discovery
Johann Dobereiner
1829 – His theory of triads
Dobereiner
2005 Q. 4 (d) (6)
He noticed that certain
elements in groups of 3
had similar physical &
chemical properties with
the atomic weight of the
middle element being
halfway between the other
two.
He called such a group of
elements a triad.
What contribution did Dobereiner make to the systematic arrangement of the elements?
(6)
Higher level only
Newlands -1864
Newland arranged all of the known
elements in order of increasing
atomic weight and he noticed the
chemical and physical properties of
the elements repeated with every 8th
element.
John Newlands
Law of octaves
He arranged the elements in order of
increasing atomic weight
John Newlands
Newlands
2006 Q. 4 (f) (6)
H
Li Be
B
C
N
O
F
Na Mg Al
Si
P
S
Every 8th known element had similar
physical & chemical properties.
What contribution did Newlands make to the systematic arrangement of the elements known to him?
(6)
Higher level only
Newlands Octaves
• The problem is that after Calcium the pattern starts to
break down.
• Although Newland had the right idea, some of the
elements hadn’t been discovered yet and this caused
elements to be forced into the wrong group!
Mendeleev and the periodic
table
Mendeleev created the first periodic table by grouping
together elements in a certain way.
Dmitri Mendeleev
1869 – He drew up the first
periodic table of the known
elements of his time by arranging
the elements in order of
increasing atomic weight.
Mendeleev
He noticed repeating patterns
which lead him to make very
accurate predictions about
undiscovered elements.
Mendeleev’s Periodic Table
No Helium
Beryllium
Hydrogen
Lithium
Carbon
Boron
- Undiscovered
H
Li
Be B C
Mendeleev’s Predictions
The differences in Mendeleev’s table and
the modern periodic table
1.
Mendeleev’s table was arranged in order of
increasing atomic mass. Modern table is
arranged in order of increasing atomic
number.
2.
In Mendeleev’s table the noble gases are
not included in the modern Table they are.
3.
There are gaps in Medeleev’s table but
there are none in the modern periodic table
as they have been discovered..
2003 Q. 4 (i) (6)
State two ways in which Mendeleev’s periodic table of the elements differs from that of Moseley.
What have you learnt about..
Dobereiner
Mendeleev
Octaves
Triads
Newlands
Henry Moseley
1913 – Henry Moseley discovered
that the positive charge in the
nucleus of an atom of any element is
of a definite amount.
These units of positive charge
became known as protons. The
periodic table is now arranged in
order of increasing atomic number.
Moseley
2008 Q. 4 (b) (6)
The atomic number of and element is the number of protons
in the nucleus of an atom of that element
Definition
What contribution did Henry Moseley, the scientist shown in the photograph,
make to the systematic arrangement
of the elements in the periodic table?
The elements in the periodic table
Today’s objectives
• Learning about Group 1 in the Periodic
Table – their properties and reactions.
Metals, non-metals or metalloids
Group 1 – The Alkali metals
Group 1 – The Alkali Metals
1.
They are all shiny
metals which are easily
cut with a knife.
2.
They all float on water
3.
They are all extremely
reactive and have to be
stored in oil to prevent
them from reacting
with the oxygen in the
air.
Demonstration – The reaction of
the alkali metals with water
1 – The reaction of lithium with water
2 – The reaction of sodium with water
3 – The reaction of potassium with
water
Explain, in terms of the structures of the atoms, the trend in reactivity down Group I (the alkali metal group) of the
periodic table.
Why do the alkali metals increase in
6
reactivity
as you go down the group?Potassium
Lithium
2006
Q. 5 (b) (9)
Sodium
As you go down the group the atomic radius
increases and the outermost electron is much
further from the nucleus and is under less of an
effect so that element is more reactive. This
outer electron is also protected from the nucleus
by an inner ‘screening effect’ of the inner
electrons.
Balanced Equations
2 Li
Lithium
2 Na
Sodium
2K
Potassium
+ 2 H2O
Water
+ 2 H2O
Water
+ 2 H2O
Water
 ½ H2
Hydrogen
 ½ H2
Hydrogen
 ½ H2
Hydrogen
+ 2 LiOH
Lithium
Hydroxide
+ 2 NaOH
Sodium
Hydroxide
+ 2 KOH
Potassium
Hydroxide
Check if you have learnt..
• What group 1 in the Table is called?
• How many electrons are in the outer shell
of group 1 elements?
• Some properties of group 1 metals?
• What happens when they are reacted with
water?
• What is the reactivity trend as you go
down the group?
In today’s class
• We will look at the properties of the rest of
the groups in the Periodic table.
Group 2 – The earth alkali metals
Includes the following elements:
Beryllium (Be)
Magnesium (Mg)
Calcium (Ca)
and others!
•They are all metals
•All of the elements in group one have two electrons in their outermost
shell!
•They are reactive- They have a tendency when reacting with outer
elements to lose these outer electrons and form ionic compounds
•They react less vigorously with water to produce hydrogen
Group 2 – The Alkaline Earth Metals
1.
They all
have 2
electrons in their outer
shell
2.
They are reactive but
not as reactive as the
alkali metals
Groups 3 -11 The d block metals
Includes the following
elements:
Scandium (Sc)
Titanium (Ti)
Vanadium (V)
Chromium (Cr)
Manganese (Mn)
Iron (Fe)
They are all metals and are
usually brightly coloured and
act as catalysts for chemical
reactions
Cobalt (Co)
Nickel (Ni)
Copper (Co)
Zinc (Zn)
and others!
Group 13
•All have 3 electrons on their outermost shell!
Group 14
Group 15
Group 16
•All have 6 electrons on their outermost shell!
•All of the group are metals except for Polonium which is a metal
Group 17 - The Halogens
•They are non metals
•All of the elements in group one
have seven electrons in their
outermost shell!
•They are reactive - They have a
tendency when reacting with
outer compounds to gain one
electron
Group 17 - The Halogens
Chlorine gas
Bromine
iodine
Group 18 - The Noble gases
They are all non metals
They are all odourless
and colourless gases
They are very
unreactive as they have
an outer shell full of
electrons, which makes
them chemically stable
Group 18 - The Noble gases
Helium gas
The odd one out.. Hydrogen